The salt cesium chloride is soluble in water. When 9.32 g CsCl is dissolved in 116,00...
The salt cesium chloride is soluble in water. When 11.9 g CsCl is dissolved in 117.00 g water, the temperature of the solution decreases from 25.00 °C to 22.56 °C. Based on this observation, calculate the dissolution enthalpy, ΔdissH, of CsCl. Assume that the specific heat capacity of the solution is 4.184 J g-1 °C-1 and that the energy transfer to the calorimeter is negligible. ΔdissH = kJ/mol
The salt sodium perchlorate is soluble in water. When 9.07 g of NaClO4 is dissolved in 103.00 g of water, the temperature of the solution decreases from 25.00 to 22.70 °C. Based on this observation, calculate the enthalpy of dissolution of NaClO4 (in kJ/mol). Assume that the specific heat of the solution is 4.184 J/g °C and that the heat absorbed by the calorimeter is negligible. ΔHdissolution kJ/mol =
When 3.90 g of cesium perchlorate (CsClO4) is dissolved in 112 g of water in a styrofoam calorimeter of negligible heat capacity, the temperature drops from 25.00 to 22.93 °C. Based on this observation, calculate q for the water and ΔH° for the process, assuming that the heat absorbed by the salt is negligible. CsClO4(s) Cs+(aq) + ClO4- (aq) The specific heat of water is 4.184 J °C-1 g-1. Give the answers in kJ. qH2O = kJ ΔH° = kJ
1. A student determines the heat of dissolution of solid magnesium chloride using a coffee-cup calorimeter of negligible heat capacity. When 0.430 g of MgCl2(s) is dissolved in 118.00 g of water, the temperature of the solution increases from 25.00 to 26.54 °C. Based on the student's observation, calculate the enthalpy of dissolution of MgCl2(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. ___?
When 4.37 g of potassium bromide (KBr) is dissolved in 109 g of water in a styrofoam calorimeter of negligible heat capacity, the temperature drops from 25.00 to 23.34 °C. Based on this observation, calculate q for the water and ΔH° for the process, assuming that the heat absorbed by the salt is negligible. KBr(s) --> K+(aq) + Br- (aq) The specific heat of water is 4.184 J °C-1 g-1.
When 3.92 g of ammonium perchlorate (NH4ClO4) is dissolved in 119 g of water in a styrofoam calorimeter of negligible heat capacity, the temperature drops from 25.00 to 22.64 °C. Based on this observation, calculate q for the water and ΔH° for the process, assuming that the heat absorbed by the salt is negligible. NH4ClO4(s) NH4+(aq) + ClO4- (aq) The specific heat of water is 4.184 J °C^-1 g^-1. Give the answers in kJ. qH2O = ______ kJ ΔH° =...
A student determines the heat of dissolution of solid cobalt(II) sulfate using a coffee-cup calorimeter of negligible heat capacity. When 1.46 g of CoSO4(s) is dissolved in 116.00 g of water, the temperature of the solution increases from 25.00 to 26.58 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoSO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. ΔHdissolution = kJ/mol
When a solid dissolves in water, heat may be evolved or absorbed. The heat of dissolution (dissolving) can be determined using a coffee cup calorimeter. In the laboratory a general chemistry student finds that when 7.79 g of CsCl(s) are dissolved in 119.70 g of water, the temperature of the solution drops from 25.48 to 23.69 °C. The heat capacity of the calorimeter (sometimes referred to as the calorimeter constant) was determined in a separate experiment to be 1.75 J/°C....
A student determines the heat of dissolution of solid copper(II) sulfate using a coffee cup calorimeter of negligible heat capacity When 2.10 g of Cus04() is dissolved in 104.00 g of water, the temperature of the solution increases from 25.00 to 27.30 °C. Based on the student's observation, calculate the enthalpy of dissolution of CuSO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 RC AH dissolution - kJ/mol
Use wie Nererences to access poi lallt values il leeueu IUI LIIS uuestivII. A student determines the heat of dissolution of solid cobalt(II) sulfate using a coffee-cup calorimeter of negligible heat capacity. When 1.63 g of CoSO4(s) is dissolved in 111.00 g of water, the temperature of the solution increases from 25.00 to 26.88 °C. Based on the student's observation, calculate the enthalpy of dissolution of CoSO4(s) in kJ/mol. Assume the specific heat of the solution is 4.184 J/g°C. AH...